Dipole-Dipole Attraction in Molecules: Analysis of BCl3, XeF4, AsH3, and SCl3

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SUMMARY

The discussion focuses on the dipole-dipole attractions in the molecules BCl3, XeF4, AsH3, and SCl3. BCl3 is identified as a neutral substance due to its trigonal planar geometry, which balances the forces. XeF4 exhibits dipole-dipole attraction due to its tetrahedral shape and lone pair, leading to an imbalanced charge. AsH3 also has dipole-dipole attraction due to its tetrahedral shape with a lone pair. SCl3 is questioned for its stability and existence, with indications that it may not be a viable compound.

PREREQUISITES
  • Understanding of molecular geometry and shapes (trigonal planar, tetrahedral).
  • Knowledge of dipole moments and polarity in molecules.
  • Familiarity with Lewis structures and electron diagrams.
  • Basic concepts of chemical bonding and molecular stability.
NEXT STEPS
  • Study the Lewis structures of AsH3 and SCl3 to understand their geometries.
  • Research the properties and stability of SCl3 and similar compounds.
  • Learn about dipole-dipole interactions in various molecular structures.
  • Explore the implications of lone pairs on molecular polarity and shape.
USEFUL FOR

Chemistry students, molecular structure researchers, and anyone interested in understanding molecular polarity and interactions in compounds.

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Homework Statement


8pFdEDX.png

http://i.imgur.com/8pFdEDX.png

Homework Equations


polarity of the element

The Attempt at a Solution


BCl3 is a trigonal planar which the forces would be balanced. Thus it is a neutral substance.
XeF4 is with tetrahedral shape where one side is a lone pair, which the charge is imbalanced and it has dipole dipole attraction between molecules.
However, I don't know the other two - AsH3 and SCl3, which one is with dipole dipole attraction between molecules? And why? Thank you very much!
 
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It is about shape of these molecules - are they symmetric enough to have a zero dipole moment?
 
A good starting point would be to draw the Lewis structures of each compound so that it's easier to figure out their geometry.
 
OK. I found AsH3 is with tetrahedral shape where one side is a lone pair, which the charge is imbalanced and it has dipole dipole attraction between molecules.

However, i can't even draw the electron diagram of SCl3. It seems there is a non-paired electron. There also no resources on SCl3 on the Internet.
The most similar structure I found is this one, SCl4. <https://upload.wikimedia.org/wikipedia/commons/2/24/Sulfur_tetrachloride.svg >
How to draw the Lewis structures of SCl3?
Thanks
 
I agree, SCl3 does not seem like it would be a stable compound. Can you check whether there was a typo in the question?
 

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